Complex Ions, Ligands, & Coordination Compounds, Basic Introduction Chemistry
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- เผยแพร่เมื่อ 29 ก.ย. 2024
- This chemistry video tutorial provides a basic introduction into complex ions, ligands, and coordination compounds. A complex ion typically consist of a transition metal cation bounded to ligands which can be neutral molecules or ions. The number of ligands attached to the transition metal ion is known as the coordination number. This video explains how to determine the oxidation state of the transition metal ion in a complex ion and within a coordination compound. A coordination compound consist of a complex ion and a counterion. The counterion may be a cation or an anion. This video briefly discusses werner's theory of coordination compounds and the concept of primary valence and secondary valence as it relates to the transition metal ions in complex ions.
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why does the 2 go at the end? Is that Algebra? pemdas? or what?
or is it the only way to make it understandable? 🤔
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He really does
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@@anetaanilnegi1801 finally someone who makes sense
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u just saved me a lot of time......tyvm...so good explanation
my chem prof gave us a 7 minute video and said good luck. thankyou for this
Thanks!
how do i tell when to use a tetrahedral or a square planar since those are the two options for a coordination number of 4?
I thought there's no lone pairs for the tetrahedral complex, but I'm probably wrong.
depends of the ligand structure i think.
It depends on how many clouds of lone electrons (electrons that aren't participating in bonds) there are. When looking at the molecular geometry is really important to count ALL electron clouds. There are two types of these, the electrons that are participating in bonding and the lone pairs of electrons.
A molecule or compound that has tetrahedral geometry has 4 electron clouds, all participating in bonding. Since all the four bonds are identical it forms a tetrahedron which is the shape that allows for all bonds to be the same.
A molecule that has square planar geometry does NOT have 4 electron clouds. In fact, it has 6 electron clouds, four of them participating in bonding and the other two are lone pair of electrons. The lone pairs have the most steric hindrance out of all the electron clouds. Because of this, the lone pairs of electrons positions themselves exactly above and below the molecule and the 4 remaining bonds have to position themselves on the "equator" of the molecule. This makes the four bonds form a square in the middle of the molecule and this is what we see.
Hope this helps.
fruitloops It depends on how many lone pairs are on the metal
If it’s sp3 (or d3s) => tetrahedral. If it’s dsp2 => sqare planar. You basically need to do the hybridation of the metal
Can you please explain covalent bond classification (MLX classes )
Thanks JG
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but what about the charge of the diamine silver cation at the beginning od the video
can some one explain it to me please ??
The amine molecules are both neutral but each has a lone pair of electrons that interact. The silver ion in the complex has a 1+ charge, so because this charge is not balanced with a 1- charge, the overall complex charge remains 1+
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Learned all of this 3 hours before my midterm. Couldn't even begin to describe what all of this was before this video. THANK YOU!!!!
For what class?
@@ayhamhuq2062 probably chemistry
Id suggest at least a day 😂
Me too,but not for a midterm, mine was for final.
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My final chemistry exam will be in 3hours from now. Transition elements. Thank you tutor
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why you donot use third bracket as it is complex !!!
I just need a friend like you for teaching me like this.
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This is also a great recap video
omg bless u this was the only video that helped understand how to differentiate the ligand types
Thanks Mark Wahlberg!
In most part of the video, you kept saying that coordination number is the number of ligands attached but it's somewhat an incorrect definition, y'know. Coordination number depends on the number of dative bonds central metal ion is attached to, so let's say if a hexadentate ligand (a molecule or ion that can form six dative bonds) attaches itself with a transition metal ion, it's coordination number will be six depending on what I said and would be one from what you have explained, which would be wrong.
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at 11:52, shouldn't you have bracketed the (CN) at the top so it looks like (CN)3? otherwise it looks like 1 carbon and 3 nitrogens.
you are the GOAT; thank you so much
I'm glad you're available on TH-cam, this is so much better than the other tutorials and I understand better
But zinc is not a transition metal, but why do we calculate the coordination number in this case.
Zinc IS a transition metal it is just ‘non-typical’ transition metal
@@amnanavid well, in our book, the definition is given that any d block metal that forms any ion which has 1-9 e- in its d orbital. but Zn doesn't seem to comply to that,so I said so
Perfect overview for my Inorganic quiz tomorrow. Good stuff 👍🏾
do we have to memorise the coordination number of each ion? I don't get how he got them from 6:55. Someone please help
I THANK YOU, your videos have really helped me with studies all throughout this and last year..
Thank you so much! You’re very clear in how you explain and were a great help to me. Hope you keep up the great work.
1:25 how do you know whether the compound is ligand just by looking at the equation.....also sir for 8:05 as the charge increases, isn't the coordination number generally decreasing? for 10:07 why did you have to draw zinc when carbon is already bonded with two oxygen atoms [or ions].......11:42 i do not see chromium having 3 atoms of it
Ligands are the groups bonded to the metal ion, so in Zn(H2O)6 2+ there are 6 H2O ligands bonded to Zn 2+
For coordination number you need to look at that data again. But it's only a general rule, you'll find transition metals form many different complexes.
He's drawing the bonds between the oxalate ion and the zinc metal...
He didn't say there's 3 atoms of Cr, look at the formula, he's saying it has a +3 charge because of the 3 x CN- counter ions.
Based on your questions I think you should watch this one again and maybe check out some other transition metal videos too.
Make upper division Inorganic Chemistry videos please.
coordination number is not the number of ligands but the number of coordinate bonds attached to the central metal ions.
Bidentate ligands bind to the central ion twice and so coordinate number will increase by two for every bidentate ligand.
i am phd physics student who has no idea about coordination chemistry nut they asked me to pass this course and i was totally lost
Thaaaaaaaaanks man u r great.
How did you even pass highschool chem?
InfiniteLoop they’re a PhD student, meaning it’s been years since they’ve been in high school let alone do high school chemistry content.
Do u have anything on Fac-mer isomers? They are in the same chapter as this one. Thanks
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This is literally the best video on complex ions, this is a waw 🤩... just lovely
Found your videos very helpful than my Uni CHEM professors' !!! Good on you, mate !!!
Good but he doesnt even explain basic logic behind ımportant things. He says, for example, when the charge increases, it makes sense that it can bind more ligangs. but why? I mean we dont really understand what type of bond is occuring here. Sorry but that is so uneducative.
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This video is more recent, longer, and more informative than my professors at MJC... Joe Caddell. He posts a 7 minute, 4 year old video, tells us it’s all we need, then gives an exam. Trash can of an effort
Sir,pls tell me that, how can I identify the situation of the ligand in complex compound??? Is it cation ,anion or neutral???
You have to add the charges from each ion, if total charge is +ve, cation, if -ve, anion and if total charge 0, it is neutral
Sir, pls tell me that, how Can i determinat the number a in this complexe {Cu(NH3)a}2+ pls help me because i have a test !!!!!!
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hey! when you talk about bidentates, you use zinc ion as an example. Zinc ion can not form a complex ion as it has a complete 3-d orbital....
Thank you very much for ur efforts so far in helping students
i had watched so many videos about this lesson but i had never seen a video like this.thnq so much for this. i hope you can make more videos like this.
I might not have time to look at the video right now (will do later) but I was wondering why the metal within complex ions was drawn with dashed bonds and the ligants still had their electron pairs draw right between the bond and the atom? Is it related to resonance form in any way or are the bonds just conventionally drawn that way? I have to ''discuss'' the metal's geometry in EDTA-Ca^2- for a lab report, it obviously looks like an octahedron but you never know.
Oh nevermind, it was just coordinate covalent bonds, I had no clue lol
Great thanks
What is the name of [Fe(CN)6]3- please?
Can anyone kindly tell me the difference between complexation and chelation
Thank you for doing all your videos with a black background
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how can Ag attached to 2 ligands since there's only 1 valence electron
6:18 this is where i get a bit confused. What dictates Td or D4h shapes
So well explained. Do you have any videos on Ligand Field Theory?
Good
Please how do we calculate the overall charge of a coordination complex
Thank you for an excellent presentation!
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Why can't the lone pairs of the other two oxygens interact ? (in the bidentate example)
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Sir can you say when the NO3 acts as counter ion
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English is not my native language so it was still pretty confusing but compeared to lecture it feels like 2+2
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